Identifying Bronsted acids and bases

[nicolely2F]

Exercise 6A.9 asks to identify which of the reactions below occur between Bronsted acids and bases. I have no problem identifying which compound is donating or accepting a proton. I'm confused on c) and d) mostly. How do I know c) isn't a Bronsted reaction? I thought it was because there is a transfer of H between CH3OOH and NH3. And then d) is a Bronsted reaction but it seems very similar to c).

a) NH4I + H2O -> NH3 + H3O+ + I-
b) NH4I -> NH3 + HI
c) CH3COOH + NH3 -> CH3CONH2 + H2O
d) NH4I + KNH2 -> KI + 2NH3

[DLee_1L]

C) and d) aren't considered bronzed-lowry reactions because there is no simple transfer of a H atom in the chemical reaction.

[nicolely2F]

C) and d) aren't considered bronzed-lowry reactions because there is no simple transfer of a H atom in the chemical reaction.

By that do you mean that in c) it isn't the H that is transferred, but the OH-?
Solutions manual says d) is a Bronsted reaction.

[DLee_1L]

Sorry, for c) yeah, its because there is an OH and NH2 swapping places. Since there's no H atom transfer, not a bronsted-lowry acid&base. For d), it is a bronsted Lowry reaction because once you separate everything into the molecules, Nh4 gives one of its h atoms to nh2. Sorry about that, didn't look at it close enough.

[nicolely2F]

Sorry, for c) yeah, its because there is an OH and NH2 swapping places. Since there's no H atom transfer, not a bronsted-lowry acid&base. For d), it is a bronsted Lowry reaction because once you separate everything into the molecules, Nh4 gives one of its h atoms to nh2. Sorry about that, didn't look at it close enough.

That explains everything, thanks a lot!